Reactivity of Metals Quiz

A list of metals arranged in order of their reactivity, from most reactive to least reactive.

The reactivity of a metal is determined by how easily it loses electrons to form positive ions. More reactive metals lose electrons more readily.

The chemical reaction between iron, oxygen, and water that forms rust (iron oxide).

A process that protects iron from rusting by coating it with a layer of zinc. Zinc is more reactive than iron and reacts with oxygen instead, preventing iron from rust.

A method of protecting iron from rusting by attaching a more reactive metal (like magnesium) that will corrode first, sacrificing itself to protect the iron.

Metals are generally higher on the reactivity series if they react violently with cold water, acids, and oxygen.

Metals higher on the reactivity series can displace metals lower on the series from their compounds. For example, zinc can displace copper from copper sulfate solution.

Metals are typically extracted from their oxides using carbon, a reducing agent that removes oxygen from the oxide. This works for metals lower in the reactivity series than carbon.

A list of elements ordered from most reactive to least reactive

A mnemonic phrase used to remember the order of metals in the reactivity series

Metals react with steam or water to produce hydrogen gas and a metal oxide

The more reactive a metal is, the more likely it is to displace another metal in a compound

The reactivity of metals in the reactivity series decreases as you move down the list

Metals placed higher in the reactivity series react with cold water, producing a metal hydroxide and hydrogen gas.

Metals in the reactivity series below calcium react with steam, producing a metal oxide and hydrogen gas.

Metals located above hydrogen in the reactivity series react with dilute acids, producing salt and hydrogen gas. The higher the metal's position, the more vigorous the reaction.

Metals like gold, silver, and copper are considered unreactive and do not react with dilute acids.

The reactivity series helps predict the products of reactions between metals and other substances.

The more reactive a metal is, the easier it will lose electrons and form positive ions.

The most reactive metals are at the top of the reactivity series, while the least reactive metals are at the bottom.

A chemical reaction that forms a salt and hydrogen gas when an acid reacts with a metal.

The higher a metal is in the reactivity series, the more vigorously it reacts. This is because they lose electrons more readily.

When a metal reacts with oxygen, it forms a metal oxide. For example, copper reacts with oxygen to form copper oxide (CuO).

Metals that are more reactive can displace metals that are less reactive from their compounds. For example, zinc can displace copper from copper sulfate solution because zinc is higher in the reactivity series.

A list that orders metals based on their reactivity, from most reactive to least reactive.

The reaction of metals with water, acids, and oxygen can tell us their relative reactivity. The more vigorous the reaction, the more reactive the metal.

The greater the temperature change during a metal's reaction with another substance, the more reactive the metal is.

Metals that react quickly or vigorously with cold water are generally higher on the reactivity series.

A protective layer of aluminium oxide that forms on the surface of aluminium, making it appear unreactive.

A process where a more reactive metal is attached to a less reactive metal to protect it from corrosion.

A process where a metal like zinc is coated onto iron to form a protective layer against corrosion.

The process where iron reacts with oxygen and water to form iron oxide (rust).

The chemical process of removing oxygen from a metal oxide using a reducing agent like carbon.

The process of a more reactive metal losing electrons and oxidizing, protecting a less reactive metal from corrosion.

Zinc reacts with oxygen and carbon dioxide in the air to form zinc carbonate, which acts as a protective barrier.

A metal higher on the reactivity series will be more likely to be oxidized and corrode first, protecting a metal lower on the series.

The coating of zinc on iron can be applied by dipping the iron into molten zinc or electroplating.

Zinc is more reactive than iron, so it will lose its electrons more easily and oxidize first, preventing iron from rusting.

If the galvanizing coating is damaged, the zinc will still protect the iron from rusting through sacrificial protection.